1. Reactions in Aqueous Solution
Chapter 4
Solution Stoich, Acid/Base theory, and Solution terms will be covered later!!!

2. Quick Review of Reactions from Chemistry I
Synthesis
Decomposition (carbonates, chlorates)
Single Replacement
Double Replacement
Combustion

3. 1. Synthesis reactions
Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.)
reactant + reactant  1 product
Basically: A + B  AB
Example: 2H2 + O2  2H2O
Example: C + O2  CO2

4. 2. Decomposition Reactions
Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds
1 Reactant  Product + Product
In general: AB  A + B
Example: 2 H2O  2H2 + O2
Example: 2 HgO  2Hg + O2

5. Decomposition Exceptions
Carbonates and chlorates are special case decomposition reactions that do not go to the elements.
Carbonates (CO32-) decompose to carbon dioxide and a metal oxide
Example: CaCO3  CO2 + CaO
Chlorates (ClO3-) decompose to oxygen gas and a metal chloride
Example: 2 Al(ClO3)3  2 AlCl3 + 9 O2
There are more exceptions!!!!!! (see handout)

6. 3. Single Replacement Reactions
Single Replacement Reactions occur when one element replaces another in a compound.
A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-).
element + compound product + product
A + BC  AC + B (if A is a metal) OR
A + BC  BA + C (if A is a nonmetal)
(remember the cation always goes first!)
When H2O splits into ions, it splits into
H+ and OH- (not H+ and O-2 !!)

7. 4. Double Replacement Reactions
Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound
Compound + compound  product + product
AB + CD  AD + CB

8. 5. Combustion Reactions
Combustion reactions occur when a hydrocarbon reacts with oxygen gas.
This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark)

9. Ionization of acetic acid
CH3COOH CH3COO- (aq) + H+ (aq)
A reversible reaction. The reaction can occur in both directions.
Acetic acid is a weak electrolyte because its ionization in water is incomplete.
4.1

10. Hydration is the process in which an ion is surrounded by water molecules arranged in a specific manner. d+ d-
H2O
4.1

11. Conduct electricity in solution?
Cations (+) and Anions (-)
Strong Electrolyte – 100% dissociation
NaCl (s) Na+ (aq) + Cl- (aq)
H2O
Weak Electrolyte – not completely dissociated
CH3COOH CH3COO- (aq) + H+ (aq)
4.1

12. Total Ionic Equations
Once you write the molecular equation (synthesis, decomposition, etc.), you should check for reactants and products that are soluble or insoluble.
We usually assume the reaction is in water
We can use a solubility table to tell us what compounds dissolve in water.
If the compound is soluble (does dissolve in water), then splits the compound into its component ions
If the compound is insoluble (does NOT dissolve in water), then it remains as a compound

13. Solubility Table from last year (say goodbye!!)

14. 4.2

15. Other Solubilities Gases only slightly dissolve in water
Strong acids and bases dissolve in water
Hydrochloric, Hydrobromic, Hydroiodic, Nitric, Sulfuric, Perchloric Acids
Group I hydroxides (in the rules already!)
Water slightly dissolves in water! (H+ and OH-)

16. Total Ionic Equations Molecular Equation:
K2CrO4 + Pb(NO3)2  PbCrO KNO3
Soluble Soluble Insoluble Soluble
Total Ionic Equation:
2 K+ + CrO Pb NO3- 
PbCrO4 (s) + 2 K+ + 2 NO3-

17. Writing Net Ionic Equations
Write the balanced molecular equation.
Write the ionic equation showing the strong electrolytes completely dissociated into cations and anions.
Cancel the spectator ions on both sides of the ionic equation
Write the net ionic equation for the reaction of silver
nitrate with sodium chloride.
AgNO3 (aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)
Ag+ + NO3- + Na+ + Cl AgCl (s) + Na+ + NO3-
Ag+ + Cl AgCl (s)
4.2

18. Net Ionic Equations
Try this one! Write the molecular, total ionic, and net ionic equations for this reaction: Silver nitrate reacts with Lead (II) Chloride in hot water
AgNO3 + PbCl2 
Molecular:
2 AgNO3 + PbCl2  2 AgCl + Pb(NO3)2
Total Ionic:
2 Ag+ + 2 NO3- + Pb Cl-  2 AgCl (s) + Pb NO3-
Net Ionic:
Ag+ + Cl-  AgCl (s)

19. Precipitation Reactions
Precipitate – insoluble solid that separates from solution
precipitate
Pb(NO3)2 (aq) + 2NaI (aq) PbI2 (s) + 2NaNO3 (aq)
molecular equation
Pb2+ + 2NO3- + 2Na+ + 2I PbI2 (s) + 2Na+ + 2NO3-
ionic equation
“If you’re not a part of the solution, then you’re a part of the precipitate!”
Pb2+ + 2I PbI2 (s)
net ionic equation
Na+ and NO3- are spectator ions
4.2

20. Chemistry In Action: - An Undesirable Precipitation Reaction
Ca2+ (aq) + 2HCO3 (aq) CaCO3 (s) + CO2 (aq) + H2O (l) -
CO2 (aq) CO2 (g)
4.2

21. Terminology for Redox Reactions
OXIDATION—loss of electron(s) by a species; increase in oxidation number; increase in oxygen.
REDUCTION—gain of electron(s); decrease in oxidation number; decrease in oxygen; increase in hydrogen.
OXIDIZING AGENT—electron acceptor; species is reduced.
REDUCING AGENT—electron donor; species is oxidized.
 When you go to a travel agent, who ends up traveling?  YOU, or the agent? 

22. You can’t have one… without the other!
Reduction (gaining electrons) can’t happen without an oxidation to provide the electrons.
You can’t have 2 oxidations or 2 reductions in the same equation. Reduction has to occur at the cost of oxidation
LEO the lion says GER!
ose
lectrons
xidation
ain
lectrons
eduction
GER!

23. Another way to remember
OIL RIG s s
xidation
eduction
ain
ose

24. Oxidation-Reduction Reactions
(electron transfer reactions)
2Mg (s) + O2 (g) MgO (s)
2Mg Mg2+ + 4e-
Oxidation half-reaction (lose e-)
O2 + 4e O2-
Reduction half-reaction (gain e-)
2Mg + O2 + 4e Mg2+ + 2O2- + 4e-
2Mg + O MgO
4.4

25. 4.4

26. Types of Oxidation-Reduction Reactions
Combination Reaction
A + B C +4 -2
S + O SO2
Decomposition Reaction
C A + B +1 +5 -2 +1 -1
2KClO KCl + 3O2
4.4

27. Types of Oxidation-Reduction Reactions
Displacement Reaction
A + BC AC + B +1 +2
Sr + 2H2O Sr(OH)2 + H2
Hydrogen Displacement +4 +2
TiCl4 + 2Mg Ti + 2MgCl2
Metal Displacement -1 -1
Cl2 + 2KBr KCl + Br2
Halogen Displacement
4.4

28. Activity Series of Metals
See handout!
lithium
potassium
strontium
calcium
sodium
magnesium
aluminum
zinc
Chromium
iron
cadmium
cobalt
nickel
tin
Lead
HYDROGEN
antimony
arsenic
bismuth
Copper
mercury
silver
palladium
Platinum gold
Each element on the list replaces from a compound any of the elements below it. The larger the interval between elements, the more vigorous the reaction.
The first five elements (lithium - sodium) are known as very active metals and they react with cold water to produce the hydroxide and hydrogen gas.
The next four metals (magnesium - chromium) are considered active metals and they will react with very hot water or steam to form the oxide and hydrogen gas.
The oxides of all of these first metals resist reduction by H2.
The next six metals (iron - lead) replace hydrogen from HCl and dil. sulfuric and nitric acids. Their oxides undergo reduction by heating with H2, carbon, and carbon monoxide.
The metals lithium - copper, can combine directly with oxygen to form the oxide.
The last five metals (mercury - gold) are often found free in nature, their oxides decompose with mild heating, and they form oxides only indirectly.

29. The Activity Series for Metals
Hydrogen Displacement Reaction
M + BC AC + B
M is metal
BC is acid or H2O
B is H2
Ca + 2H2O Ca(OH)2 + H2
Pb + 2H2O Pb(OH)2 + H2
Figure 4.15
4.4

30. Types of Oxidation-Reduction Reactions
Disproportionation Reaction
Element is simultaneously oxidized and reduced. +1 -1
Cl2 + 2OH ClO- + Cl- + H2O
Chlorine Chemistry
4.4

31. Chemistry in Action: Breath Analyzer+6
3CH3CH2OH + 2K2Cr2O7 + 8H2SO4 +3
3CH3COOH + 2Cr2(SO4)3 + 2K2SO4 + 11H2O
4.4

32. Zn (s) + CuSO4 (aq) ZnSO4 (aq) + Cu (s)
Zn Zn2+ + 2e-
Zn is oxidized
Zn is the reducing agent
Cu2+ + 2e Cu
Cu2+ is reduced
Cu2+ is the oxidizing agent
Copper wire reacts with silver nitrate to form silver metal.
What is the oxidizing agent in the reaction?
Cu (s) + 2AgNO3 (aq) Cu(NO3)2 (aq) + 2Ag (s)
Cu Cu2+ + 2e-
Ag+ + 1e Ag
Ag+ is reduced
Ag+ is the oxidizing agent
4.4

33. Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2
Oxidation number
The charge the atom would have in a molecule (or an
ionic compound) if electrons were completely transferred.
Free elements (uncombined state) have an oxidation number of zero.
Na, Be, K, Pb, H2, O2, P4 = 0
In monatomic ions, the oxidation number is equal to the charge on the ion.
Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2
The oxidation number of oxygen is usually –2. In H2O2 and O22- it is –1.
4.4

34. HCO3- O = -2 H = +1 3x(-2) + 1 + ? = -1 C = +4
The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1.
Group IA metals are +1, IIA metals are +2 and fluorine is always –1.
6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion.
HCO3-
Oxidation numbers of all the elements in HCO3- ?
O = -2
H = +1
3x(-2) ? = -1
C = +4
4.4

35. Figure 4.10 The oxidation numbers of elements in their compounds
4.4

36. IF7 F = -1 7x(-1) + ? = 0 I = +7 K2Cr2O7 NaIO3 Na = +1 O = -2 O = -2
Oxidation numbers of all the elements in the following ?
F = -1
7x(-1) + ? = 0
I = +7
K2Cr2O7
NaIO3
Na = +1
O = -2
O = -2
K = +1
3x(-2) ? = 0
7x(-2) + 2x(+1) + 2x(?) = 0
I = +5
Cr = +6
4.4

37. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus
fruits contain citric acid.
Cause color changes in plant dyes.
React with certain metals to produce hydrogen gas.
2HCl (aq) + Mg (s) MgCl2 (aq) + H2 (g)
React with carbonates and bicarbonates to produce carbon
dioxide gas
2HCl (aq) + CaCO3 (s) CaCl2 (aq) + CO2 (g) + H2O (l)
Aqueous acid solutions conduct electricity.
4.3

38. Bases Have a bitter taste. Feel slippery. Many soaps contain bases.
Cause color changes in plant dyes.
Aqueous base solutions conduct electricity.
4.3

39. Neutralization Reaction
acid + base salt + water
HCl (aq) + NaOH (aq) NaCl (aq) + H2O
H+ + Cl- + Na+ + OH Na+ + Cl- + H2O
H+ + OH H2O
4.3

40. New AP format (2007) Equations must be balanced
Questions will be asked about the reaction (descriptive?)
Example:
4. For each of the following three reactions, in part (i) write a BALANCED equation and in part (ii) answer the question about the reaction. In part (i), coefficients should be in terms of lowest whole numbers. Assume that solutions are aqueous unless otherwise indicated. Represent substances in solutions as ions if the substances are extensively ionized. Omit formulas for any ions or molecules that are unchanged by the reaction. Example: A strip of magnesium is added to a solution of silver nitrate.
(i) Mg + 2 Ag + → Mg Ag (ii) Which substance is oxidized in the reaction? Answer: Magnesium (Mg) metal